1. correct
2. reconsider some of the choices, noting that the volume is increased, so decide which side will be favoured by additional volume.
Please tell me if these are right.
1.According to Le Chatelier’s principle, what is the effect on the products when N2 is added to the equilibrium mixture of each of the following reactions?
a. 2NH3(g) < = > 3H2(g) + N2(g)
B. N2(g) + O2(g) <= > 2NO(g)
C. 2NO2(g)< => N2(g) +2O2(g)
D. 4NH3(g) + 3O2(g) <= > 2N2(g) +6H2O(g)
A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products
2.Would increasing the volume of the equilibrium mixture of each of the following reactions cause the equilibrium to shift and if so will the shift be toward products or reactants.
a. 2NH3(g) < => 3H2(g) + N2(g)
B. N2(g) +O2(g) <= > 2NO(g)
C. 2NO2(g) <= > N2(g) + 2O2(g)
D. 4NH3(g) +3O2(g) <= > 2N2(g) + 6H2O(g)
A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products
2 answers
1.
A. equilibrium shifts to reactants
agreed
B. equilibrium shifts to products
agreed
C. equilibrium shifts to reactants
agreed
D. equilibrium shifts to products
Reactants?
2.
A. equilibrium shifts to reactants
No
B. equilibrium shifts to products
No
C. equilibrium shifts to reactants
No
D. equilibrium shifts to products
agreed
For part 2 if the pressure was increased then the equilibrium shifts in such a way as to oppose the change, i.e. will shift to a smaller volume. As moles are equivalent to volume then you can read these as e.g. equation A
2 mole => 4 moles. So increasing the pressure will move the equilibrium towards the reactants.
In the case of incareasing the volume, the pressure must decrease, so the equilibrium will shift in the opposite direction to a pressure increase. That is to a larger total volume, so the equilibria will shift in the direction that has the larger number of moles.
For equation A
2 mole => 4 moles. So decreasing the pressure or increasing the volume will move the equilibrium towards the products.
A. equilibrium shifts to reactants
agreed
B. equilibrium shifts to products
agreed
C. equilibrium shifts to reactants
agreed
D. equilibrium shifts to products
Reactants?
2.
A. equilibrium shifts to reactants
No
B. equilibrium shifts to products
No
C. equilibrium shifts to reactants
No
D. equilibrium shifts to products
agreed
For part 2 if the pressure was increased then the equilibrium shifts in such a way as to oppose the change, i.e. will shift to a smaller volume. As moles are equivalent to volume then you can read these as e.g. equation A
2 mole => 4 moles. So increasing the pressure will move the equilibrium towards the reactants.
In the case of incareasing the volume, the pressure must decrease, so the equilibrium will shift in the opposite direction to a pressure increase. That is to a larger total volume, so the equilibria will shift in the direction that has the larger number of moles.
For equation A
2 mole => 4 moles. So decreasing the pressure or increasing the volume will move the equilibrium towards the products.